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Secondary Cells

Which of the ...

Question

Which of the following is TRUE in case of recharging a Lead Storage Battery?

A

P b S O_{4} (s) + 2 e^{-} \to P b (s) + S O_{4}^{2 -} (a q)

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B

P b S O_{4} (s) + 2 H_{2} O \to P b O_{2} (s) + S O_{4}^{2 -} (a q) + 4 H^{+} (a q) + 2 e^{-}

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C

P b (s) + S O_{4}^{2 -} (a q) \to P b S O_{4} (s) + 2 e^{-}

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D

P b O_{2} (s) + S O_{4}^{2 -} + 4 H^{+} (a q) + 2 e^{-} \to P b S O_{4} (s) + 2 H_{2} O (l)

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Solution

The correct options are
A $P b S O_{4} (s) + 2 e^{-} \to P b (s) + S O_{4}^{2 -} (a q)$
B $P b S O_{4} (s) + 2 H_{2} O \to P b O_{2} (s) + S O_{4}^{2 -} (a q) + 4 H^{+} (a q) + 2 e^{-}$
During recharging, the cell operates like an electrolytic cell, i.e., now electrical energy is supplied to it from an external source. The electrode reactions are the reverse of those that occur during discharge:
$P b S O_{4} (s) + 2 e^{-} \to P b (s) + S O_{4}^{2 -} (a q)$
$P b S O_{4} (s) + 2 H_{2} O \to P b O_{2} (s) + S O_{4}^{2 -} (a q) + 4 H^{\oplus} (a q) + 2 e^{-} 2 P b S O_{4} (s) + 2 H_{2} O \to P b (s) + P b O_{2} (s) + 4 H^{\oplus} (a q) + 2 S O_{4}^{2 -} (a q)$
Such operation is possible because PbSO₄ formed during discharge is a solid and sticks to the electrodes. It is, therefore, in a position to either receive or give up electrons during electrolysis.

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Similar questions

Q. During the discharge of a lead storage battery, density of

H_{2} S O_{4}

1.294

1.139

. S u l p h u r i c a c i d o f d e n s i t y

i s

b y w e i g h t a n d t h a t o f d e n s i t y

i s

b y w e i g h t . T h e b a t t e r y h o l d

o f t h e a c i d a n d v o l u m e r e m a i n s p r a c t i c a l l y c o n s t a n t d u r i n g d i s c h a r g e . C a l c u l a t e a m p e r e - h o u r o f w h i c h t h e b a t t e r y m u s t h a v e b e e n u s e d . T h e c h a r g i n g a n d d i s c h a r g i n g r e a c t i o n s a r e :

Pb + SO_{4}^{2-} \rightarrow PbSO_{4} + 2e^{-}

(c h a r g i n g)

PbO_{2} + 4H^{+} + SO_{4}^{2-} + 2e^{-}\rightarrow PbSO_{4} + 2H_{2}O$ (discharging).

Q. The standard reduction potential at STP

(25^{\circ} C

and 1 atm) of the following half cells are found as below.

P b_{a q}^{2 +} + 2 e^{-} \to P b_{(s)} E^{0} = - 0.121 V P b O_{2 (s)} + 4 H_{(a q)}^{+} + S O_{4 (a q)}^{2 -} + 2 e^{-} \to P b S O_{4 (s)} + 2 H_{2} O E^{0} = 1.71 V P b_{(a q)}^{4 +} + 2 e^{-} \to P b_{(a q)}^{2 +} E^{0} = 1.689 V

P b S O_{4 (s)} + 2 e^{-} \to P b_{(s)} + S O_{4 (a q)}^{2 -}

E^{0}

is missing but it is found that in an aqueous solution of

H_{2} S O_{4}

having a pH=1.7, when

P b S O_{4 (s)}

is put, then at saturated condition
Solubility of

P b S O_{4} = 5 \times 10^{- 5} M o l / L

(T a k e \frac{2.303 R T}{F} = 0.06 a n d l o g 2 = 0.3)

List-I contains questions and List-II contains their answers.

\begin{matrix} List-I & List-II What is the E^{0} (in V) for the half-cell (I) P b S O_{4 (s)} + 2 e^{-} \to P b_{(s)} + S O_{4 (a q)}^{2 -} ? & (P) -0.168 What is the E_{c e l l}^{0} (in V) of a lead storage battery? It has (II) the cell reaction as P b_{(s)} + P b O_{2 (s)} + 2 H_{2} S O_{4_{(a q)}} \to 2 P b S O_{4 (s)} + 2 H_{2} O_{(l)} & (Q) 0.7 What is the E^{0} (in V) for the half cell (III) P b O_{2 (s)} + 4 H_{(a q)}^{+} + 4 e^{-} \to P b_{(s)} + 2 H_{2} O_{(I)} & (R) 2.0 K_{s p} is the equilibrium constant for the reaction (IV) P b O_{2 (s)} + 4 H_{(a q)}^{+} ⇌ P b_{(a q)}^{4 +} + 2 H_{2} O_{(l)} & (S) -0.068 What is the value of E^{o} (in V) ? (T) -0.31 (U) 2.02 \end{matrix}

Which of the following options has the correct combination considering the reactions in List-I and their answers in List-II?

Q. The standard reduction potential at STP

(25^{\circ} C

and 1 atm) of the following half cells are found as below.

P b_{a q}^{2 +} + 2 e^{-} \to P b_{(s)} E^{0} = - 0.121 V P b O_{2 (s)} + 4 H_{(a q)}^{+} + S O_{4 (a q)}^{2 -} + 2 e^{-} \to P b S O_{4 (s)} + 2 H_{2} O E^{0} = 1.71 V P b_{(a q)}^{4 +} + 2 e^{-} \to P b_{(a q)}^{2 +} E^{0} = 1.689 V

P b S O_{4 (s)} + 2 e^{-} \to P b_{(s)} + S O_{4 (a q)}^{2 -}

E^{0}

is missing but it is found that in an aqueous solution of

H_{2} S O_{4}

having a pH=1.7, when

P b S O_{4 (s)}

is put, then at saturated condition
Solubility of

P b S O_{4} = 5 \times 10^{- 5} M o l / L

(T a k e \frac{2.303 R T}{F} = 0.06 a n d l o g 2 = 0.3)

List-I contains questions and List-II contains their answers.

\begin{matrix} List-I & List-II What is the E^{0} (in V) for the half-cell (I) P b S O_{4 (s)} + 2 e^{-} \to P b_{(s)} + S O_{4 (a q)}^{2 -} ? & (P) -0.168 What is the E_{c e l l}^{0} (in V) of a lead storage battery? It has (II) the cell reaction as P b_{(s)} + P b O_{2 (s)} + 2 H_{2} S O_{4_{(a q)}} \to 2 P b S O_{4 (s)} + 2 H_{2} O_{(l)} & (Q) 0.7 What is the E^{0} (in V) for the half cell (III) P b O_{2 (s)} + 4 H_{(a q)}^{+} + 4 e^{-} \to P b_{(s)} + 2 H_{2} O_{(I)} & (R) 2.0 K_{s p} is the equilibrium constant for the reaction (IV) P b O_{2 (s)} + 4 H_{(a q)}^{+} ⇌ P b_{(a q)}^{4 +} + 2 H_{2} O_{(l)} & (S) -0.068 What is the value of E^{o} (in V) ? (T) -0.31 (U) 2.02 \end{matrix}

Which of the following options has the correct combination considering the reactions in List-I and their answers in List-II?

Q. The standard reduction potential at STP

(25^{\circ} C

and 1 atm) of the following half cells are found as below.

P b_{a q}^{2 +} + 2 e^{-} \to P b_{(s)} E^{0} = - 0.121 V P b O_{2 (s)} + 4 H_{(a q)}^{+} + S O_{4 (a q)}^{2 -} + 2 e^{-} \to P b S O_{4 (s)} + 2 H_{2} O E^{0} = 1.71 V P b_{(a q)}^{4 +} + 2 e^{-} \to P b_{(a q)}^{2 +} E^{0} = 1.689 V

P b S O_{4 (s)} + 2 e^{-} \to P b_{(s)} + S O_{4 (a q)}^{2 -}

E^{0}

is missing but it is found that in an aqueous solution of

H_{2} S O_{4}

having a pH=1.7, when

P b S O_{4 (s)}

is put, then at saturated condition
Solubility of

P b S O_{4} = 5 \times 10^{- 5} M o l / L

(T a k e \frac{2.303 R T}{F} = 0.06 a n d l o g 2 = 0.3)

List-I contains questions and List-II contains their answers.

\begin{matrix} List-I & List-II What is the E^{0} (in V) for the half-cell (I) P b S O_{4 (s)} + 2 e^{-} \to P b_{(s)} + S O_{4 (a q)}^{2 -} ? & (P) -0.168 What is the E_{c e l l}^{0} (in V) of a lead storage battery? It has (II) the cell reaction as P b_{(s)} + P b O_{2 (s)} + 2 H_{2} S O_{4_{(a q)}} \to 2 P b S O_{4 (s)} + 2 H_{2} O_{(l)} & (Q) 0.7 What is the E^{0} (in V) for the half cell (III) P b O_{2 (s)} + 4 H_{(a q)}^{+} + 4 e^{-} \to P b_{(s)} + 2 H_{2} O_{(I)} & (R) 2.0 K_{s p} is the equilibrium constant for the reaction (IV) P b O_{2 (s)} + 4 H_{(a q)}^{+} ⇌ P b_{(a q)}^{4 +} + 2 H_{2} O_{(l)} & (S) -0.068 What is the value of E^{o} (in V) ? (T) -0.31 (U) 2.02 \end{matrix}

Which of the following options has the correct combination considering the reactions in List-I and their answers in List-II?

Q. The standard reduction potential at STP

(25^{\circ} C

and 1 atm) of the following half cells are found as below.

P b_{a q}^{2 +} + 2 e^{-} \to P b_{(s)} E^{0} = - 0.121 V P b O_{2 (s)} + 4 H_{(a q)}^{+} + S O_{4 (a q)}^{2 -} + 2 e^{-} \to P b S O_{4 (s)} + 2 H_{2} O E^{0} = 1.71 V P b_{(a q)}^{4 +} + 2 e^{-} \to P b_{(a q)}^{2 +} E^{0} = 1.689 V

P b S O_{4 (s)} + 2 e^{-} \to P b_{(s)} + S O_{4 (a q)}^{2 -}

E^{0}

is missing but it is found that in an aqueous solution of

H_{2} S O_{4}

having a pH=1.7, when

P b S O_{4 (s)}

is put, then at saturated condition
Solubility of

P b S O_{4} = 5 \times 10^{- 5} M o l / L

(T a k e \frac{2.303 R T}{F} = 0.06 a n d l o g 2 = 0.3)

List-I contains questions and List-II contains their answers.

\begin{matrix} List-I & List-II What is the E^{0} (in V) for the half-cell (I) P b S O_{4 (s)} + 2 e^{-} \to P b_{(s)} + S O_{4 (a q)}^{2 -} ? & (P) -0.168 What is the E_{c e l l}^{0} (in V) of a lead storage battery? It has (II) the cell reaction as P b_{(s)} + P b O_{2 (s)} + 2 H_{2} S O_{4_{(a q)}} \to 2 P b S O_{4 (s)} + 2 H_{2} O_{(l)} & (Q) 0.7 What is the E^{0} (in V) for the half cell (III) P b O_{2 (s)} + 4 H_{(a q)}^{+} + 4 e^{-} \to P b_{(s)} + 2 H_{2} O_{(I)} & (R) 2.0 K_{s p} is the equilibrium constant for the reaction (IV) P b O_{2 (s)} + 4 H_{(a q)}^{+} ⇌ P b_{(a q)}^{4 +} + 2 H_{2} O_{(l)} & (S) -0.068 What is the value of E^{o} (in V) ? (T) -0.31 (U) 2.02 \end{matrix}

Which of the following options has the correct combination considering the reactions in List-I and their answers in List-II?

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